2 g of `FeC_(2)O_(4)` are made to react in acid solution with `0.25 M KMnO_(4)` solution. What volume of `KMnO_(4)` would be required? The be reqruied? The resulting solution is treated with excess of `NH_(4)Cl` solution and `NH_(4)OH` solution. The precipitated `Fe(OH)_(3)` is filtered off, washed and ignited. What is the mass of the product obtained? (Atomic weight of `Fe=56`)

Explanation

To solve the problem step by step, we will first determine the volume of KMnO4 required to react with 2 g of FeC2O4, and then calculate the mass of Fe(OH)3 obtained after the subsequent reactions.

### Step 1: Calculate the number of moles of FeC2O4

The molar mass of FeC2O4 (Iron(II) oxalate) can be calculated as follows:
- Atomic weight of Fe = 56 g/mol
- Atomic weight of C = 12 g/mol (2 Carbon atoms)
- Atomic weight of O = 16 g/mol (4 Oxygen atoms)
...